Answer : The final volume of a gas is,
Explanation :
According to the Charles's law, the volume of a gas is directly proportional to the temperature of the gas at constant pressure and the number of moles of gas.
or,
where,
= initial volume of gas =
= final volume of gas = ?
= initial temperature of gas = 491 K
= final temperature of gas = 297 K
Now put all the given values in the above formula, we get the final volume of a gas.
Therefore, the final volume of a gas is,
Answer:
The type of reaction for the following equation is combustion equation.
Explanation:
Combustion reaction is defined as the chemical reaction in which a hydrocarbon reacts with oxygen gas to produce carbon dioxide gas and water molecule.
The reaction given to us:
When 1 mole of ethane reacts with 7/2 moles of oxygen gas it gives 3 moles of water and 2 moles of carbon dioxide gas.
The type of reaction for the following equation is combustion equation.
Answer:
percent yield = 40.6 %
Explanation:
The question asks to determine the percent yield, which can be defined as:
percent yield =
where the actual yield is how much product was obtained, in this case 12.5 g of CCl₂F₂, and the theoretical yield is how much product could be obtained with the given reactants theoretically.
So we know already the actual yield, we need to <em>calculate the theoretical yield.</em>
First we need to <em>write the reaction chemical equation</em>:
CCl₄ + HF → CCl₂F₂ + HCl
and <em>balance the equation</em>:
CCl₄ + 2 HF → CCl₂F₂ + 2 HCl
In the equation we can see that <em>for every mol of CCl₄ we should get 1 mol of CCl₂F₂</em> (molar ratio 1:1). So if we <u>calculate the moles of CCl₄</u> in the given 39.2 g of CCl₄ we could know how many moles of CCl₂F₂ (assuming HF is in excess).
From the molar ratio we know:
Moles of CCl₂F₂ = moles of CCl₄ = 0.2549 moles
Now we need to <u>convert these moles into grams</u> to get the theoretical yield of CCl₂F₂ in grams:
Percent yield = (12.5 g / 30.81 g) * 100 = 40.6 %